Question 1

Indicate which of the following plots would be obtained for a second-order reaction.

Accepted Answer

A)   
B)   
C)   
D)

Question 2

The rate of a reaction is found to double when the concentration of one reactant is quadrupled. The order of the reaction with respect to this reactant is __________

Accepted Answer

A)   first.
B)   second.
C)   one-quarter.
D)   one-half.
E)   third.

Question 3

Given the following data for the reaction A  B, determine the frequency factor, A, of the reaction. k (M/s) 
T (°C) 
0) 282
277
0) 291
627

Accepted Answer

A)   +0.304
B)   +1.31
C)   +1.19
D)   +0.270
E)   -0.500

Question 4

When one chemical is a precursor of another chemical in a series of reactions, the concentrations of the two species are said to be __________

Accepted Answer

A)   catalytic.
B)   volatile.
C)   coalescent.
D)   linked.
E)   intermediate.

Question 5

A catalyst that is in a different phase from the reactants and products is a __________ catalyst.

Accepted Answer

A)   heterogeneous
B)   homogeneous
C)   enzyme-type
D)   protein
E)   exogenous

Question 6

Which point as labeled by an asterisk (*)  on the following energy profile is the transition state?

Accepted Answer

A)   
B)   
C)   
D)

Question 7

Which of these could be the units for the rate constant in a second-order reaction?

Accepted Answer

A)   M-1 s
B)   M s-1
C)   M-1 s-1
D)   M-2 s-1
E)   Ms

Question 8

The steps in a reaction mechanism are as follows. Which species is acting as a catalyst? Step 1: Ag+(aq)  + Ce4+(aq)   Ag2+(aq)  + Ce3+(aq) 
Step 2: Tl+(aq)  + Ag2+(aq)   Tl2+(aq)  + Ag+(aq) 
Step 3: Tl2+(aq)  + Ce4+(aq)   Tl3+(aq)  + Ce3+(aq)

Accepted Answer

A)   Ag+
B)   Tl+
C)   Ce3+
D)   Ag2+
E)   Tl3+

Question 9

A reaction mechanism consists of a series of __________ steps.

Accepted Answer

A)   molecular
B)   primary
C)   steric
D)   elementary
E)   secondary

Question 10

The linear form of the Arrhenius equation is very useful, as a plot of ln k vs. 1/T allows us to calculate the activation energy from the __________ and the frequency factor from the __________.

Accepted Answer

The answer of The linear form of the Arrhenius equation...

Question 11

The reaction NO2(g)  + CO(g)   NO(g)  + CO2(g)  is thought to occur by the following mechanism: Step 1: NO2(g)  + NO2(g)   NO3(g)  + NO(g) 
Step 2: NO3(g)  + CO(g)   NO2(g)  + CO2(g) 
Which of the following species is an intermediate?

Accepted Answer

A)   NO2
B)   NO
C)   NO3
D)   CO2
E)   This mechanism has no intermediates.

Question 12

The following graph shows the kinetics curves for the reaction of oxygen with hydrogen to form water: O2(g)  + 2H2(g)   2H2O(g) . Which curve is hydrogen? 2(g)  + 2H2(g)   2H2O(g) . Which curve is hydrogen?   A)  the dashed curve B)  the gray curve C)  the black curve D)  either the gray or the black curve E)  Any of these curves could be hydrogen." class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   the dashed curve
B)   the gray curve
C)   the black curve
D)   either the gray or the black curve
E)   Any of these curves could be hydrogen.

Question 13

Which of the following is not important as a contributing factor to photochemical smog?

Accepted Answer

A)   stagnant air
B)   sunlight
C)   lots of traffic
D)   irrigation
E)   cars without catalytic converters

Question 14

Which of the following describes a reaction mechanism?
(I) Consists of a series of elementary steps
(II) Reproduces the experimentally determined rate law
(III) Is the way the reaction actually occurs

Accepted Answer

A)   I only
B)   III only
C)   II only
D)   I and II only
E)   I, II, and III

Question 15

The mechanism for the first-order reaction 2H2O2(aq)   2H2O( 2O2(aq)   2H2O(   )  + O2 in the presence of I-(aq)  is proposed to be Step 1: H2O2(aq)  + I-(aq)   H2O(   )  + OI-(aq)  (slow)  Step 2: H2O2(aq)  + OI-(aq)   H2O(   )  + O2(g)  + I-(aq)  (fast)  Identify the catalyst in the reaction. A)  H2O2 B)  OI- C)  I- D)  H2O E)  O2" class="answers-bank-image d-inline" rel="preload" > )  + O2 in the presence of I-(aq)  is proposed to be
Step 1: H2O2(aq)  + I-(aq)   H2O( 2O2(aq)   2H2O(   )  + O2 in the presence of I-(aq)  is proposed to be Step 1: H2O2(aq)  + I-(aq)   H2O(   )  + OI-(aq)  (slow)  Step 2: H2O2(aq)  + OI-(aq)   H2O(   )  + O2(g)  + I-(aq)  (fast)  Identify the catalyst in the reaction. A)  H2O2 B)  OI- C)  I- D)  H2O E)  O2" class="answers-bank-image d-inline" rel="preload" > )  + OI-(aq) 
(slow) 
Step 2: H2O2(aq)  + OI-(aq)   H2O( 2O2(aq)   2H2O(   )  + O2 in the presence of I-(aq)  is proposed to be Step 1: H2O2(aq)  + I-(aq)   H2O(   )  + OI-(aq)  (slow)  Step 2: H2O2(aq)  + OI-(aq)   H2O(   )  + O2(g)  + I-(aq)  (fast)  Identify the catalyst in the reaction. A)  H2O2 B)  OI- C)  I- D)  H2O E)  O2" class="answers-bank-image d-inline" rel="preload" > )  + O2(g)  + I-(aq) 
(fast) 
Identify the catalyst in the reaction.

Accepted Answer

A)   H2O2
B)   OI-
C)   I-
D)   H2O
E)   O2

Question 16

Which of the following does the initial rate of a chemical reaction depend on?
(I) Concentration of reactants
(II) Concentration of products
(III) Temperature

Accepted Answer

A)   I
B)   III
C)   II
D)   Both I and III
E)   I, II, and III

Question 17

The reaction 2NO(g)  + O2(g)   2NO2(g)  has the following rate law: Rate = k[O2][NO]2. If the concentration of NO is reduced by a factor of two, the rate will __________

Accepted Answer

A)   double.
B)   quadruple.
C)   be reduced by one-quarter.
D)   be reduced by one-half.
E)   remain the same.

Question 18

The following energy profiles for four different reactions are shown. Which reaction is the most exothermic?

Accepted Answer

A)   a
B)   b
C)   c
D)   d

Question 19

For the rate law Rate = k[A]1/2[B], the partial order with respect to A is __________, the partial order with respect to B is __________, and the total order is __________.

Accepted Answer

Question 20

For the reaction 2A + 3B F1F1F1S1F1F1F10 4C + 5D, the rate of the reaction in terms of F1F1F1S1F1F1F10C would be written as __________.

Accepted Answer

+ <img  loading="lazy" src="/assets/images/blured-textbook.svg" class="d-inline m-1" alt="blured image" width="139" height="30"> F1F1F1S...

Exam 15: Chemical Kinetics

Which point as labeled by an asterisk (*) on the following energy profile is the transition state?

Correct AnswerverifiedShow Answer

The rate of a reaction is found to double when the concentration of one reactant is quadrupled. The order of the reaction with respect to this reactant is __________

Correct AnswerverifiedShow Answer

The linear form of the Arrhenius equation is very useful, as a plot of ln k vs. 1/T allows us to calculate the activation energy from the __________ and the frequency factor from the __________.

Correct AnswerverifiedShow Answer

Which of the following describes a reaction mechanism? (I) Consists of a series of elementary steps (II) Reproduces the experimentally determined rate law (III) Is the way the reaction actually occurs

Correct AnswerverifiedShow Answer

The following graph shows the kinetics curves for the reaction of oxygen with hydrogen to form water: O2(g) + 2H2(g)  2H2O(g) . Which curve is hydrogen?

Correct AnswerverifiedShow Answer

The following energy profiles for four different reactions are shown. Which reaction is the most exothermic?

Correct AnswerverifiedShow Answer

For the reaction 2A + 3B  4C + 5D, the rate of the reaction in terms of C would be written as __________.

Correct Answerverified+ F1F1F1S...View AnswerShow Answer

A catalyst that is in a different phase from the reactants and products is a __________ catalyst.

Correct AnswerverifiedShow Answer

Which of these could be the units for the rate constant in a second-order reaction?

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Given the following data for the reaction A  B, determine the frequency factor, A, of the reaction. k (M/s) T (°C) 0) 282 277 0) 291 627

Correct AnswerverifiedShow Answer

Which of the following does the initial rate of a chemical reaction depend on? (I) Concentration of reactants (II) Concentration of products (III) Temperature

Correct AnswerverifiedShow Answer

Which of the following is not important as a contributing factor to photochemical smog?

Correct AnswerverifiedShow Answer

A reaction mechanism consists of a series of __________ steps.

Correct AnswerverifiedShow Answer

The reaction 2NO(g) + O2(g)  2NO2(g) has the following rate law: Rate = k[O2][NO]2. If the concentration of NO is reduced by a factor of two, the rate will __________

Correct AnswerverifiedShow Answer

The mechanism for the first-order reaction 2H2O2(aq)  2H2O( ) + O2 in the presence of I-(aq) is proposed to be Step 1: H2O2(aq) + I-(aq)  H2O( ) + OI-(aq) (slow) Step 2: H2O2(aq) + OI-(aq)  H2O( ) + O2(g) + I-(aq) (fast) Identify the catalyst in the reaction.

Correct AnswerverifiedShow Answer

The steps in a reaction mechanism are as follows. Which species is acting as a catalyst? Step 1: Ag+(aq) + Ce4+(aq)  Ag2+(aq) + Ce3+(aq) Step 2: Tl+(aq) + Ag2+(aq)  Tl2+(aq) + Ag+(aq) Step 3: Tl2+(aq) + Ce4+(aq)  Tl3+(aq) + Ce3+(aq)

Correct AnswerverifiedShow Answer

Indicate which of the following plots would be obtained for a second-order reaction.

Correct AnswerverifiedShow Answer

When one chemical is a precursor of another chemical in a series of reactions, the concentrations of the two species are said to be __________

Correct AnswerverifiedShow Answer

For the rate law Rate = k[A]1/2[B], the partial order with respect to A is __________, the partial order with respect to B is __________, and the total order is __________.

Correct AnswerverifiedShow Answer

The reaction NO2(g) + CO(g)  NO(g) + CO2(g) is thought to occur by the following mechanism: Step 1: NO2(g) + NO2(g)  NO3(g) + NO(g) Step 2: NO3(g) + CO(g)  NO2(g) + CO2(g) Which of the following species is an intermediate?

Correct AnswerverifiedShow Answer

Correct Answer
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Correct Answer
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The linear form of the Arrhenius equation is very useful, as a plot of ln k vs. 1/T allows us to calculate the activation energy from the and the frequency factor from the .

Correct Answer
verified

Correct Answer
verified

The following graph shows the kinetics curves for the reaction of oxygen with hydrogen to form water: O₂(g) + 2H₂(g)  2H₂O(g) . Which curve is hydrogen?

Correct Answer
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Correct Answer
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Correct Answer
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+ F1F1F1S...
View Answer

Correct Answer
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Correct Answer
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The reaction 2NO(g) + O₂(g)  2NO₂(g) has the following rate law: Rate = k[O₂][NO]². If the concentration of NO is reduced by a factor of two, the rate will __________

Correct Answer
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The mechanism for the first-order reaction 2H₂O₂(aq)  2H₂O( ) + O₂ in the presence of I^-(aq) is proposed to be Step 1: H₂O₂(aq) + I^-(aq)  H₂O( ) + OI^-(aq) (slow) Step 2: H₂O₂(aq) + OI^-(aq)  H₂O( ) + O₂(g) + I^-(aq) (fast) Identify the catalyst in the reaction.

Correct Answer
verified

The steps in a reaction mechanism are as follows. Which species is acting as a catalyst? Step 1: Ag⁺(aq) + Ce⁴⁺(aq)  Ag²⁺(aq) + Ce³⁺(aq) Step 2: Tl⁺(aq) + Ag²⁺(aq)  Tl²⁺(aq) + Ag⁺(aq) Step 3: Tl²⁺(aq) + Ce⁴⁺(aq)  Tl³⁺(aq) + Ce³⁺(aq)

Correct Answer
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Correct Answer
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For the rate law Rate = k[A]^1/2[B], the partial order with respect to A is , the partial order with respect to B is , and the total order is __.

Correct Answer
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The reaction NO₂(g) + CO(g)  NO(g) + CO₂(g) is thought to occur by the following mechanism: Step 1: NO₂(g) + NO₂(g)  NO₃(g) + NO(g) Step 2: NO₃(g) + CO(g)  NO₂(g) + CO₂(g) Which of the following species is an intermediate?

Correct Answer
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